The black tarnish that forms on silver objects is primarily Ag.S. The half reaction for reversing the tarnishing process is as follows: a. Predict which of the following can reduce Ag.S to Ag under standard condition (Use data from the Standard Reduction Potential table) • H;Oza • Zne) Sn b. Of those mentioned in (a), identify which is the strongest reducing agent in aqueous solution and thus best candidate for a commercial product c. Suggest an alternative reducing agent that is readily available, inexpensive, and possibly more effective at removing tarnish (Use data from the Standard Reduction Potential table)

indTap - Cengage Learni.. Courses Transfer Course Equivalen. OWLV2 | Online teaching Homepage [Review Topics] [References] Use the References to access important values if needed for this question. Use standard reduction potentials to calculate the equilibrium constant for the reaction: Hg*(aq) + 2I°(aq)→ Hg(1) + I½(s) Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant: AG° for this reaction would be O than zero. Submit Answer Retry Entire Group 9 more group attempts remaining Previou Email Instruc Cengage Learning | Cengage Technical Support DII DD F9 F10 F11 F4 ES F6 F7 F8 F3 $ % & 4 5 6 7 8 9

Known standard reduction potential data for: Cd2+ + 2e → Cd E° = -0,40 V Cr3* + 3e > Cr E° = -0,74 V Based on these data, which of the following statements is true... A. Cd is a stronger reducing agent than Cr B. At the anode oxidation occurs Cd to Cd2+ C. The electrochemical cell potential that occurs is 0.34 V D. If the two half-cell reactions are linked, then Cr3+ will be reduced to Cr

Which of the following compounds is the greatest oxidizing agent using the standard reduction potentials below?         a.    MnO2 (s)     b.    Hg (l)     c.    SnO2 (s)     d.    Cr(OH)3 (s)

V. OWLV2 | Online teaching and leaX takeCovalentActivity.do?locator3Dassignment-take Update ロ * 。 [Review Topics] [References] Use the References to access important values if needed for this question. ba bə Use standard reduction potentials to calculate the standard free energy change in k] for the reaction: (M) Ni2*(aq) + Hg(1)– Ni(s) + Hg2"(aq) bə. bə. K for this reaction would be than one. bəj Retry Entire Group 8 more group attempts remaining Submit Answer bəj VD 10:51 PM 5/16/2022 直 +6 国星 C

OWLV2 | Online teaching and le + keCovalentActivity.do?locator=assignment-take Update : [Review Topics] [References) Use the References to access important values if needed for this question. eq Use standard reduction potentials to calculate the standard free energy change in k] for the reaction: eq 2(s) + H2(g)21(aq) + 2H*(aq) req Answer: kJ K for this reaction would be than one. Visited 2req Submit Answer Retry Entire Group 8 more group attempts remaining 2req 11:24 PM 2 63°F 5/16/2022

A concentration cell similar to the one shown is composed of two Sn electrodes and solutions of different Sn2+ concentrations. The left compartment contains 0.974 M Sn2+ , and the right compartment contains 0.677 M Sn2+ .Calculate the cell potential for this reaction at 298 K. volts In this tin concentration cell, the compartment on the left is the    , and the compartment on the right is the    .

A chromium metal was deposited coming from a solution of Cr+3. The amount of the saidmetal deposited weighs 2.19 g. The process is made possible through a current of 35.2Amperes in electrolyte cell. Determine the following:a. How much charge (in C) is required?b. How long (in min) would it take for the reaction to occur?